500 mL of 0.1019 M NaOH solution is left open immediately after preparation, and it absorbs 0.652 g CO2. Calculate the relative carbonate error made in acetic acid titration with this solution with phenol-phthalate indicator.

500 mL of 0.1019 M NaOH solution is left open immediately after preparation, and it absorbs 0.652 g CO2. Calculate the relative carbonate error made in acetic acid titration with this solution with phenol-phthalate indicator.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter21: Potentiometry

Section: Chapter Questions

Problem 21.12QAP

See similar textbooks

Related questions

Q: Enumerate at least 3 specific medical applications of complexometric titration and discuss each.

A: The ligand is a species that contains an unshared electron pair or a negative charge. This electron…

Q: Write two features of Erichrome black- T which makes it a suitable indicator in complexometric…

A: Two features of Eriochrome black- T has to be written The medium it undergoes complex formation has…

Q: A 250.0-mg sample of an organic weak acid was dissolved in an appropriate solvent and titrated with…

A: Assuming the equivalent weight of acid is E. Given : mass of acid = 250 mg = 0.25 g…

Q: An indicator was not used during potentiometric titration of a weak acid Is there a positive…

A: A question based on potentiometric titration that is to be accomplished.

Q: An indicator with an acid dissociation constant of 2.19 x 10‑5 could typically be used for a…

A: The question is based on the concept of titration. it involves the application of indicator. we…

Q: Calculate the percentage mass of the possible alkaline component/s.

Q: A 39.3 mL aliquot of ammonia that has a concentration of 0.655 M will be titrated with 0.304 M HCl.…

Q: exist? 4. What makes bromocresol green and phenolphthalein suitable for the double- indicator…

A: 4. The pH value of phenolphthalein ranges between 8.3 to 10. which makes it suitable as double…

Q: Iodometric titration of vitamic C with sodium thiosulfate Why was the known excess of iodine…

A: Ascorbic acid (vitamin C) is mainly found in fresh fruits such as lemon, orange, lime, peach,…

Q: Use the titration curve for the weak acid to calculate the pH of a 0.150 M solution of that weak…

A: The pKa of the acid will be equal to the pH at half equivalence point which can be determined by…

Q: For the titration: 30.0mL of 0.150 M NH3 (Kb = 1.8 x 10-5) with 0.250 M HBr Calculate the pH after…

A: For the given titration we have to calculate the pH

Q: encountered during the analysis in double indicator titration (determining of carbonates in a…

Q: If you weighed out 0.2194 g of pure KHP for your exploratory titration with the NaOH solution and it…

A: Given: 0.2194 g of pure KHP 23.51 mL of NaOH

Q: true or false 1.,Carbonic acid, as a contaminant in the assay of sodium bicarbonate, may render…

A: Methyl orange is used as an indicator in this titration.

Q: In compleximetric titration, why should the conditional formation constant between the indicator and…

A: In complexometric titration, the metal ion concentration is determined with the help of a…

Q: 13. What is the pH range should be maintained in an argentometric titration for the estimation of…

A: This method determines the chloride ion conc. of a solution by titration with AgNO3. As the AgNO3…

Q: 25.00 mL of 0.35 M sulphuric acid, H2SO4 was titrated with 0.75 M ammonia, NH3. Illustrate a…

A: 25 ml x 0.35 M of H2SO4 =8.75mmoles NH3 =0.75M inital pHinital pH is determined by H2SO4H2SO4→KA1…

Q: Generate a curve for the titration of 30.00mL of a solution in which the analytical concentration of…

A: The titration curve of an acid base titration is the plot of the pH of the reaction mixture with the…

Q: 00 mL of 0,1019 m NaOH solution prepared immediately after, the lid is left open and absorbs 0.652 g…

A: Molarity of NaOH after standardization = 0.1019 M Volume of NaOH=500.0 mL Mass of CO2 absorbed by…

Q: After preparing 500 mL of 0.1019 M NaOH solution, the cap is left open and it absorbs 0.652 g CO2.…

Q: Discuss the theory behind potentiometric pH determinations. Then compare the advantages and…

A: Potentiometric pH meter is used to measure the difference in electric potential between the pH…

Q: Ethanol is needed as solvent when preparing phenolphthalein color indicator in volumetric…

A: Ethanol - class of alcohol containing 2 carbons and 1 alcoholic group and it is a industrial…

Q: Why homogenously formed precipitates are better suited for analysis than a precipitate formed by…

A: The gravimetric method is inherently more accurate than the volumetric method because the…

Q: What is selective precipitation? What is confirmatory test and its significance? What are the…

A: In selective precipitation only specifically the one which is desired is precipitated in presence of…

Q: Question attached

A: EDTA is ethylene diamine tetra acetic acid. It is a hexadentate ligand. The ability of multidentate…

Q: In the determination of Mass% NaOCI in Bleach Sample (Titration), does addition of water to the…

A: During the mass % determination of NaOCl in bleach sample, first NaOCl is converted to HOCl in…

Q: What factor affects the ‘strength’ of a buffer? Why was benzoic acid used as a solvent when making…

A: Firstly we have to tell about factor affecting the strength of a buffer solution. Ratio of…

Q: In which cases are the wet Electorstatic Precipitators used?

A: In which cases are the wet Electrostatic Precipitators used?

Q: 500 ml of 0.1019 M NaOH solution is prepared It is immediately forgotten with the cap open and…

A: NaOH reacts with carbon dioxide as: 2NaOH+CO2→Na2CO3+H2O

Q: Condition of permanganatometric titration of sodium oxalate includes: pH = 1 and heating of analyte…

A: Permanganatometric titration is a technique used in chemical quantitative analysis. It is a type of…

Q: What is a 3 point calibration in titration?

A: Detail about 3 point calibration in titration is given below.

Q: Would the indicator bromocresol green, with a transition range of pH 3.8–5.4, ever be useful in the…

A: weak acid react with strong base, it give basic solution. So, the pH of the solution after…

Q: A chemist adds enough of the theoretical ionic compound MX3 to form a saturated solution. She knows…

A: One mole of MX3 will dissociates into 1 mole of M3+ and 3 mol X-. Let the solubility of MX3 be “s”

Q: Explain the reason behind the addition of the starch indicator near the endpoint for this analysis.…

A: Starch is an indicator used in iodometric titration and it turns dark blue when iodine is present in…

Q: 2) The following experimental process steps have been made to determine the hardness of water.…

A: Hard water does not form lather with soap instead from a curd-like substance. It is due to the…

Q: The titration of a polyprotic acid with sufficiently different pKa ’s displays two equivalence…

A: Polyprotic acid produces two different H+ ions upon ionization like diprotic acid.

Q: The following experimental process steps have been made to determine the hardness of water.…

A: The hardness of water is the result of the presence or the formation of a curd-like substance when…

Q: True or False Very Insoluble precipitates are not the best candidates for gravimetric analysis.

A: In order for the analysis to be accurate, The ion being analyzed must be completely precipitated.…

Q: The titration curve from the reaction of a strong base with a weak acid is shown below. Recalling…

Q: If 2 mL of 0.02 M AgNO3 is added to 2 mL 0.011 M K2CrO4, which reagent is in excess? should a…

A: Solution- 2mL of 0.02 M agNO3-2mL ×0.02 mol L=0.04 M mol AgNO32mL of 0.0011 M K2CrO4-2mL ×…

Q: I did an experiment called Potentiometric Analyses where we titrate NaOH with a solid unknown weak…

A: 2 mole of OH- neutralizes 1 mole of acid Formula used : Molarity = no. of moles/vol(Lt)

Q: What is the importance of having a titration of about pH 10 in compleximetric titration?

A: In complexometric titration end point is observed by the formation coloured complex.

Q: What are the effects produced by photo composition on an improperly stored standard solution of…

A: Since the end point does not exactly coincide with the equivalence point, the titrant should the…

Q: Titration of 0.1 M HCl against a 25mL liquor mixture of NaOH and Na2CO3 using phenolphthalein…

Q: Calculate the relative carbonate error made in acetic acid titration

A: According to question Concentration of NaOH = 0.1019M Volume of NaOH = 0.5L No. Of moles of NaOH…

Q: Complexometric titration must be performed at pH 10.0

A: Complexometric Titration is basically a type of volumetric titration where a colored complex is…

Q: Why is bromophenol blue and not phenolphthalein used as an indicator for the antacid titration?

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Concept explainers

Precipitation Titration

Precipitation analysis is used to analyze drugs, and to measure the salt content in food and beverages. It is an important concept from the examination point of view many practical questions are asked on the topic. This topic is significant in the professional exams for both undergraduate and graduate courses, especially for

Question

100%

500 mL of 0.1019 M NaOH solution is left open immediately after preparation, and it absorbs 0.652 g CO₂. Calculate the relative carbonate error made in acetic acid titration with this solution with phenol-phthalate indicator.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 4 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

After preparing 500 mL of 0.1019 M NaOH solution, the cap is left open and it absorbs 0.652 g CO2. With this solution, Calculate the relative carbonate error in acetic acid titration besides the phenol phthalate indicator.
Write two features of Erichrome black- T which makes it a suitable indicator in complexometric titration. In which medium does it undergo complex formation?
500 mL of 0.1019 M NaOH solution is preparedIt is immediately forgotten with the cap open and absorbs 0, 652 g of CO2. Calculate the relative carbonate error made in acetic acid titration with this solution with phenol-phthalate indicator.
Why are the standard reagents used in neutralization titrations generally strong acids and bases ratherthan weak acids and bases? Explain.
An indicator was not used during potentiometric titration of a weak acid Is there a positive error, negative error, no effect, or error could not be determined In terms of the Computed pKa of the unknown weak acid?
Titration of 0.1 M HCl against a 25mL liquor mixture of NaOH and Na2CO3 using phenolphthalein indicator requires 17.5mL of the acid for the endpoint. After this, methyl orange was added and 3.5mL of HCl was again required for the next endpoint. A. Write separate equations for reactions for the two endpoints B. Calculate the amount in milligrams of NaOH and Na2CO3 in the mixture
In the experiment of the acid dissociation constant of a weak acid using potentiometric titration, what primary standard was used to standardize NaOH in this experiment? Give the appropriate equation for the reaction.
Would the indicator bromocresol green, with a transition range of pH 3.8–5.4, ever be useful in the titration of a weak acid with a strong base? Why?
If water was used to rinse the conical flask used for the titration, how would this affect your final estimate of hydrochloric acid concentration? (More, less or unchanged?) Explain why, discussing the number of moles that you would actually have due to the rinsing
In which cases are the wet Electorstatic Precipitators used?
What is a 3 point calibration in titration?
true or false 1.,Carbonic acid, as a contaminant in the assay of sodium bicarbonate, may render the end point to be yellow. 2,.To have a balanced equation in the assay of sodium bicarbonate, the titrant should have a coefficient of one and the sulfate salt of sodium produced should have a coefficient of three. 3.When a weak alkali is titrated with strong acid, the indicator used is methyl red.4 4.Sodium bicarbonate is considered as the primary standard in its own assay. 5.When a strong alkali is titrated with a strong acid, phenolphthalein may be used.